A saturated solution of iodine in water contain 0.330g I_(2) per litre. More than this I_(2) can be dissolved in KI solution because of the following equilibrium. I_(2(g))+I^(-)hArrI_(3)^(-) A 0.100 M KI solution actually dissolves 12.5 g "iodine per litre", most of which is converted to I_(3)^(-). Assuming that the concentration of I_(2) in all saturated solution is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated solution of I_(2) in the KI solution?

A saturated solution of iodine in water contain 0.330g I_(2) per litre

1.	A saturated solution of iodine in water contain 0.330g I_(2) per litre. More than this I_(2) can be dissolved in KI solution because of the following equilibrium. I_(2(g))+I^(-)hArrI_(3)^(-) A 0.100 M KI solution actually dissolves 12.5 g "iodine per litre", most of which is converted to I_(3)^(-). Assuming that the concentration of I_(2) in all saturated solution is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated solution of I_(2) in the KI solution?
Answer» <html><body><p></p><a href="https://interviewquestions.tuteehub.com/tag/solution-25781" style="font-weight:bold;" target="_blank" title="Click to know more about SOLUTION">SOLUTION</a> :`707 <a href="https://interviewquestions.tuteehub.com/tag/litre-1075864" style="font-weight:bold;" target="_blank" title="Click to know more about LITRE">LITRE</a> <a href="https://interviewquestions.tuteehub.com/tag/mol-1100196" style="font-weight:bold;" target="_blank" title="Click to know more about MOL">MOL</a>^(-<a href="https://interviewquestions.tuteehub.com/tag/1-256655" style="font-weight:bold;" target="_blank" title="Click to know more about 1">1</a>)` ,</body></html>